Organic Chemistry 1 Review

Front 1

What is Organic Chemistry?

Back 1

Chemistry of compounds containing carbon.

Front 2

Inorganic Chemistry

Back 2

Chemistry of compounds not containing carbon.

Front 3

What is the simplest organic compound?

Back 3

Methane: CH4

Front 4

Three ways to represent organic compounds are?

Back 4

1. Condensed structural formula
2. Dash Formula
3. Bond-Line formula

Front 5

CH3CH2CH2CH2CH3 is an example of what kind of representation?

Back 5

Condensed n-pentane

Front 6

Functional Groups:

What are Alkanes?

Back 6

Carbon-Carbon Single Bond

Ex. 2-methylpentane

Front 7

What are Alkenes?

Back 7

(Olefins)
carbon--carbon double bond

Ex. 1-octene

Front 8

What are Alkynes?

Back 8

Carbon---Carbon Triple bond

Ex. 4-octyne

Front 9

What are Aromatics?

Back 9

(Arenes)
Cyclic compound triple bonded to another.
Ex. Benzene

Front 10

What are Haloalkanes?

Back 10

Alkyl halides,
carbon-Halogen Bond

Ex. 3-chloroheptane

Front 11

What are Alcohols?

Back 11

Carbon-Oxygen Hydrogen Bond

Ex. Ethanol

Front 12

What are Ethers?

Back 12

Carbon-Oxygen-Carbon bond

Ex. Diethyl Ether

Front 13

What are Amines?

Back 13

A Nitrgoen being bonded to Carbon or hydrogen

Ex. Diethyl Amine

Front 14

What are Aldehydes?

Back 14

A double bonded Oxygen bonded to just one carbon, on one side. (Hydrogen may be on other side)

Ex. 3-methylhexanal

Front 15

What are Ketones?

Back 15

A double bonded Oxygen bonded to just two carbons, one on each sides.

Ex. 2-Decanone

Front 16

What are Carboxylic Acids?

Back 16

A double bonded Oxygen bonded to just one carbon, on one side and an OH group on the other side.

Ex. Propanoic acid

Front 17

What are Esters?

Back 17

A double bonded Oxygen bonded to just one carbon, on one side and an oxygen bonded to a carbon on the other side.

Ex. Ethyl Butanoate

Front 18

What are Amides?

Back 18

A double bonded Oxygen bonded to just one carbon, on one side, a nitrogen on the other side bonded to two carbons. (carbon could be a hydrogen)

Ex. 7-methyl octanamide

Front 19

What are Nitriles?

Back 19

A carbon bonded to another carbon, which is then triple bonded to a Nitrogen.

Ex. 2-methylpentanenitrile

Front 20

What is an Empirical Formula?

Back 20

A chemical formula that shows the kinds of atoms and their RELATIVE numbers in a substance.

Front 21

What is a Molecular Formula?

Back 21

A chemical formula that indicates the ACTUAL number of atoms of each element in one molecule of a substance.

Front 22

What is the Molecular and Empirical formula of Ethylene?

Back 22

Molecular: C2H2

Empirical: CH2

Front 23

What is the Molecular and Empirical formula of cyclohexane?

Back 23

Molecular: C6H12

Empirical: CH2

Front 24

What is the Molecular and Empirical formula of 1-pentene?

Back 24

Molecular: C5H10

Empirical: CH2

Front 25

Structural Theory of Organic Chemistry:

What are the two central fundamental premises?

Back 25

1)The atoms of the elements in organic compounds can form a fixed # of bonds. The measure of this ability is called VALENCE.
Ex. Carbon is tetravalent; that is carbon atoms form "4" bonds.
Oxygen is divalent; oxygen atoms form "2" bonds.
Hydrogen and the halogens are monovalent; their atoms only form one bond.

2)A carbon atom can use one or more of its valences to form bonds to other carbon atoms.

Front 26

What is an Isomer?

Back 26

Different compounds that have the same molecular formula. There are many types of isomers.

Front 27

Constitutional Isomer?

Back 27

Different compounds that have the same molecular formula, but differ in their connectivity, that is, the sequence in which their atoms are bonded together.

Ex. Ethyl alcohol and dimethyl ether.

Front 28

What is Saturation?

Back 28

Carbon with max. amount of hydrogen attached to them. (alkanes)

Front 29

What is Unsaturation?

Back 29

Carbons with out the max. amount of hydrogens attached to them.

Always compared with the parent alkane.

Front 30

Units of Saturation are AKA?

Back 30

Double bond equivalents (DBE)
Index of Hydrogen deficiency(IHD)

Front 31

Double bonds = __ units of Saturation?

Back 31

1 unit

Front 32

Cyclic Compounds = __ units of Saturation?

Back 32

1 unit

Front 33

Triple bonds = __ units of Saturation?

Back 33

2 units

Front 34

Aromatic rings = __ units of Saturation?

Back 34

4 units (1 for the ring, 3 for each double bond)

Front 35

What is the equation for finding the units of unsaturation?

Back 35

Units Unsat.=
((2)(#C)+2)-((#H)-(#X)+(#N))
---------------------------
2

*Ignore Oxygen

Front 36

What is the Units of Saturation in C4H10?

Back 36

0 units

Front 37

What is the Units of Saturation in CH3CH2CH2CH3?

Back 37

0 units

Front 38

What is the Units of Saturation in butane(C4H8)?

Back 38

1 unit

Front 39

What are Ionic Bonds?

Back 39

Formed by the transfer of one or more electrons from one atom to another to create ions (ionic bonds are formed between metal and a non-metal).

Front 40

What is a covalent bond?

Back 40

A bond that is formed when the two atoms share electrons (covalent bonds are formed between non-metals).

Front 41

What is the Octet Rule?

Back 41

Bonded atoms tend to possess or share a total of eight valence-shell electrons.

Front 42

What are the exceptions to the Octet Rule?

Back 42

1)Elements of the 3rd period and beyond, have "d" orbital for bonding. These elements can accomodate more than eight electrons in their valence shell and therefore can form more than four covalent bonds.

Ex. PCL5 and SF6

2) Some highly reactive molecules or ons have atoms with fewer than eight electrons in their outer shell.

Ex. BH3 and BX3 (X=Halogen)

Front 43

What is a formal charge?

Back 43

The unit positive or negative charge of atom in a molecule or ion (formal charges are integers, ie. +1, 0, -2, etc.)

Front 44

The arithmetic sum of all of the formal charges of each atom equals the ____ ____ (also and integer) on the molecule or ion.

Back 44

total charge

Front 45

What equation is used to calculate the formal charge?

Back 45

FC= Z-A

Z= Number of valence electrons it has at a neutral free atom (group #)

A= Number of valence electrons assigned to an atom in its boned state.

Front 46

The total charge on the ion or molecule is calculated by adding all what?

Back 46

The formal charges of each atom within the ion or molecule.

Front 47

Ions always have a total charge other than ____.

Back 47

Zero

Front 48

Molecules always have a total charge of ____ .

Back 48

Zero

Front 49

What is Resonance stuctures?

Back 49

Individual Lewis structures in cases where two or more lewis structures are equally good descriptions of a single molecule or ion. The individual resonance structures in such an instance are "averaged" to give a correct description of the real molecule or ion.

Front 50

What is the Resonance theory?

Back 50

This theory states that whenever a molecule or ion can be represented by two or more lewis structures that differ only in the position of the electrns, two things will be true.

1. None of the individual strutures, which we term "resonance structures," will be a correct representation for the molecule or ion. NONE will be in complete accord with the physical and chemical properties of the substance.

2. The actual molecule or ion will be better represented by a "resonance hybrid" of these structures.

Front 51

What is an orbital?

Back 51

A region of space where the probabilty of finding an electron is large.

Front 52

What is a node?

Back 52

An area of space where the probabilty of finding an electron is zero. Think of a "p" orbital. Also remeber the greater the number of nodes, the greater the energy.

Front 53

What is the Pauli Exclusion Principle?

Back 53

No two electrons can have the same four quantum #'s!!
Better Defn: A max. of two electrons may be placed in each orbital but only when the spins of the electrons are paired. We designate paired electrons as ( ). Unpaired electrons, which are not permitted in the same orbital, are designated as ( ) or ( ). Think of the three 2p orbitals (degenerate orbitals).

Front 54

What are the 4 quantum numbers?

Back 54

n(principle quantum #): 0 to infinity

l(angular momentum quantum #): 0 to n-l

m (magnetic quantum #): l to 0 to +l

*All three of these quantum #'s are always integers*

s(spin quantum #): (+1/2 or
-1/2)

Front 55

What is Aufbau Principle?

Back 55

Orbitals are filled up so that those of lowest energy are filled first.

Front 56

What is Hund's Rule?

Back 56

When we come to orbitals of equal energy (degenrate orbital) such as the three "p" orbital, we add one electron to each with their spins unpaired until each degenerate orbital contains one electron, then, we begin adding a second electron to each degenerate orbital so that the spins are paired.

Front 57

What is the Heinsenburg Uncertainty principle?

Back 57

We CANNOT know simultaneously the position and momentum of an electron. That is, we cannot pin down the electrons as precisely as our explanation suggests.

Front 58

What are Atomic Orbitals (AO's)?

Back 58

A region of space around an atom where the probability of finding an electron is large.

Front 59

What are Molecular Orbitals (MO's)?

Back 59

A region of space within a molecule where the probability of finding an electron is large.